practice exam3 - C Suppose[A(0 = 1...

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A. Calculate the equilibrium constant K for the reaction: 2NO(g) + O 2 (g) = 2NO 2 (g) at P = 1 atm, T = 298K using the following data: compound G f 0 , kJ/mol H f 0 , kJ/mol NO 86.606 90.291 NO 2 51.258 33.095 B. Will the equilibrium constant increase or decrease if temperature is increased? Explain your answer. C. Calculate the equilibrium constant for P=100 atm and T = 298K. Assume that the reactants and the product are ideal gases. D. Suppose you have initially 1 mole of NO, 1 mole of O 2 and 1 mole of NO 2 . At a later moment, the amount of NO 2 was found to be 1.2 mol. What are the amounts of NO and O 2 at the same time?
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2. In the reaction mechanism shown below k 1 = k -1 = 1 s -1 , k 2 = k -2 = 2 s -1 , k 3 = k -3 =3 s -1 , k 4 = 4 s -1 , k = 3.1416 s -1 . A. What is k -4 ? B . Write the differential equations for the time evolution of [B] and [E].
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Unformatted text preview: C . Suppose [A](0) = 1 mol/l, [B](0)=[C](0)=[D](0)=[E](0)=0. What will be the final concentrations [A]( ∞ ) and [E] ( ∞ )? Answer the same question in the case where k = 0. 3. A dimerization 2A Ø A 2 is found to be a first order process. To explain this surprising result the following mechanism has been proposed: k 1 A Ø A * k 2 A * + A Ø A 2 where k 2 >> k 1 . A. Assuming that one can use the steady state approximation for A * , find [A * ] and obtain the rate expressions for [A 2 ] and [A] . B. The half-life t 1/2 of a reaction is the time required for half of the reactant (A) to disappear. What is the half-life of the above reaction?...
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